What is a mole, anyway? Chemists define a mole as a collective unit that represents6.02 x 10 ^ 23 particles of a substance. Since twenty-one zeros are hard to process, compare the term "mole" to the words "dozen" or "couple." Each are just names for a specific number.
And molar mass? The average atomic mass of an element (expressed in grams) is the molar mass. For example, Gallium's molar mass would be approximately 70 grams because its atomic mass is 69.723 g.
Calculating Compounds Figuring out the molar mass of a compound is very similar; a little dimensional analysis is involved, but it all begins with calculating the molar mass of each individual element in the formula.
If there are two or more atoms of a certain element, simply multiply its molar mass by however many atoms there are. Let's try NH3 (Ammonia). Click the link below for a step-by-step demo, and check out our two videos for a more in-depth explanation.
Mole-to-Mass Conversion Mole-to-mass conversion is very important, because an experiment may require an exact number of grams (not moles) of a substance. Refer to this equation once you've determined the molar mass of your substance.
What is a mole, anyway?
Chemists define a mole as a collective unit that represents 6.02 x 10 ^ 23 particles of a substance. Since twenty-one zeros are hard to process, compare the term "mole" to the words "dozen" or "couple." Each are just names for a specific number.
And molar mass?
The average atomic mass of an element (expressed in grams) is the molar mass. For example, Gallium's molar mass would be approximately 70 grams because its atomic mass is 69.723 g.
Calculating Compounds
Figuring out the molar mass of a compound is very similar; a little dimensional analysis is involved, but it all begins with calculating the molar mass of each individual element in the formula.
If there are two or more atoms of a certain element, simply multiply its molar mass by however many atoms there are. Let's try NH3 (Ammonia). Click the link below for a step-by-step demo, and check out our two videos for a more in-depth explanation.
What is the mass of 90 average sized apples[1].doc
molar mass of glucose[1].doc
And don't forget about significant digits!
Find more videos like this on Hill's Chemistry 1 Wiki Developers
Find more videos like this on Hill's Chemistry 1 Wiki Developers
Mole-to-Mass Conversion
Mole-to-mass conversion is very important, because an experiment may require an exact number of grams (not moles) of a substance. Refer to this equation once you've determined the molar mass of your substance.
mass (grams) = number of moles x mass (grams)
1 mol
Find more videos like this on Hill's Chemistry 1 Wiki Developers